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Chemistry / Chemistry: A Molecular Approach 3 / Chapter 4 / Problem 88E

Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro

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A 30.00 mL sample of an unknown H3PO4 solution is titrated

Chapter 4, Problem 88E

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QUESTION:

A 30.00 mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.38 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution? The neutralization reaction is

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QUESTION:

A 30.00 mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.38 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution? The neutralization reaction is

ANSWER:

Solution: Here, we are going to write a balanced chemical equation for the given reaction and calculate the concentration of the remaining ions. Also, we are going to determine whether the resultant solution is acidic or basic. Step1: a) When a solution of 15.0 g of Sr(OH) is mixed with 2solution of 255.0 ml of 0.200 M HN0 , strontium nitrate and water are formed. The balanced chemical equation for the 3 above reaction is given below: Sr(OH) (a2 + 2HN0 (aq) --3---> Sr(N0 ) (aq) + 23 2 2 Step2: b) Given mass of Sr(OH) = 15.0 g 2 Molar mass of Sr(OH) = 121.6 g/ mol 2 Therefore, number of moles of Sr(OH) = 15.0 / 121

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